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Acids and Bases

Acids and Bases. Acid/Base Definitions. Arrhenius Model Acids produce hydrogen ions in aqueous solutions Bases produce hydroxide ions in aqueous solutions Bronsted-Lowry Model Acids are proton donors Bases are proton acceptors Lewis Acid Model Acids are electron pair acceptors

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Acids and Bases

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  1. Acids and Bases

  2. Acid/Base Definitions • Arrhenius Model • Acids produce hydrogen ions in aqueous solutions • Bases produce hydroxide ions in aqueous solutions • Bronsted-Lowry Model • Acids are proton donors • Bases are proton acceptors • Lewis Acid Model • Acids are electron pair acceptors • Bases are electron pair donors

  3. Acid Dissociation HA (aq) H+(aq) + A- (aq) AcidProtonConjugate base Alternately, H+ may be written in its hydrated form, H3O+ (hydronium ion)

  4. Dissociation of Strong Acids Strong acids are assumed to dissociate completely in solution. Large Ka or small Ka? Reactant favored or product favored?

  5. Dissociation Constants: Strong Acids

  6. Dissociation of Weak Acids Weak acids are assumed to dissociate only slightly (less than 5%) in solution. Large Ka or small Ka? Reactant favored or product favored?

  7. Dissociation Constants: Weak Acids

  8. Self-Ionization of Water H2O + H2O  H3O+ + OH- At 25, [H3O+] = [OH-] = 1 x 10-7 Kw is a constant at 25 C: Kw = [H3O+][OH-] Kw = (1 x 10-7)(1 x 10-7) = 1 x 10-14 = [Ka][Kb]

  9. pH and pOH Calculations

  10. pH Scale

  11. Calculating pH, pOH pH = -log10(H3O+) pOH = -log10(OH-) Relationship between pH and pOH pH + pOH = 14 Finding [H3O+], [OH-] from pH, pOH [H3O+] = 10-pH [OH-] = 10-pOH

  12. A Weak Acid Equilibrium Problem What is the pH of a 0.50 M solution of acetic acid, HC2H3O2, Ka = 1.8 x 10-5 ? Step #1:Write the dissociation equation HC2H3O2 C2H3O2- + H+

  13. A Weak Acid Equilibrium Problem What is the pH of a 0.50 M solution of acetic acid, HC2H3O2, Ka = 1.8 x 10-5 ? Step #2:ICE it! HC2H3O2 C2H3O2- + H+ 0.50 0 0 +x +x - x x x 0.50 - x

  14. A Weak Acid Equilibrium Problem What is the pH of a 0.50 M solution of acetic acid, HC2H3O2, Ka = 1.8 x 10-5 ? Step #3:Set up the law of mass action HC2H3O2 C2H3O2- + H+ E 0.50 - x x x

  15. A Weak Acid Equilibrium Problem What is the pH of a 0.50 M solution of acetic acid, HC2H3O2, Ka = 1.8 x 10-5 ? Step #4:Solve for x, which is also [H+] HC2H3O2 C2H3O2- + H+ E 0.50 - x x x [H+] = 3.0 x 10-3 M

  16. A Weak Acid Equilibrium Problem What is the pH of a 0.50 M solution of acetic acid, HC2H3O2, Ka = 1.8 x 10-5 ? Step #5:Convert [H+] to pH HC2H3O2 C2H3O2- + H+ E 0.50 - x x x pH = - log (3.0 x 10-3) = 2.52

  17. Dissociation of Strong Bases MOH(s)  M+(aq) + OH-(aq) • Strong bases are metallic hydroxides • Group I hydroxides (NaOH, KOH) are very soluble • Group II hydroxides (Ca, Ba, Mg, Sr) are less soluble • pH of strong bases is calculated directly from the concentration of the base in solution

  18. Reaction of Weak Bases with Water The base reacts with water, producing its conjugate acid and hydroxide ion: CH3NH2 + H2O  CH3NH3+ + OH- Kb = 4.38 x 10-4

  19. Kb for Some Common Weak Bases Many students struggle with identifying weak bases and their conjugate acids.What patterns do you see that may help you?

  20. Reaction of Weak Bases with Water The generic reaction for a base reacting with water, producing its conjugate acid and hydroxide ion: B + H2O  BH+ + OH-

  21. A Weak Base Equilibrium Problem What is the pH of a 0.50 M solution of ammonia, NH3, Kb = 1.8 x 10-5 ? Step #1:Write the equation for the reaction NH3 + H2O  NH4+ + OH-

  22. A Weak Base Equilibrium Problem What is the pH of a 0.50 M solution of ammonia, NH3, Kb = 1.8 x 10-5 ? Step #2:ICE it! NH3 + H2O  NH4+ + OH- 0.50 0 0 +x +x - x x x 0.50 - x

  23. A Weak Base Equilibrium Problem What is the pH of a 0.50 M solution of ammonia, NH3, Kb = 1.8 x 10-5 ? Step #3:Set up the law of mass action NH3 + H2O  NH4+ + OH- E 0.50 - x x x

  24. A Weak Base Equilibrium Problem What is the pH of a 0.50 M solution of ammonia, NH3, Kb = 1.8 x 10-5 ? Step #4:Solve for x, which is also [OH-] NH3 + H2O  NH4+ + OH- E 0.50 - x x x [OH-] = 3.0 x 10-3 M

  25. A Weak Base Equilibrium Problem What is the pH of a 0.50 M solution of ammonia, NH3, Kb = 1.8 x 10-5 ? Step #5:Convert [OH-] to pH NH3 + H2O  NH4+ + OH- E 0.50 - x x x pOH = - log (3.0 x 10-3) = 2.52 pH = 14 - pOH = 11.48

  26. Acid-Base Properties of Salts These salts simply dissociate in water: KCl(s)  K+(aq) + Cl-(aq)

  27. Acid-Base Properties of Salts The basic anion can accept a proton from water: C2H3O2- + H2O  HC2H3O2 + OH- base acid acid base

  28. Acid-Base Properties of Salts The acidic cation can act as a proton donor: NH4+(aq)  NH3(aq) + H+(aq) Acid Conjugate Proton base

  29. Acid-Base Properties of Salts • IF Ka for the acidic ion is greater than Kb for the basic ion, the solution is acidic • IF Kb for the basic ion is greater than Ka for the acidic ion, the solution is basic • IF Kb for the basic ion is equal to Ka for the acidic ion, the solution is neutral

  30. Acid-Base Properties of Salts Step #1: AlCl3(s) + 6H2O  Al(H2O)63+(aq) + Cl-(aq) Salt water Complex ion anion Step #2: Al(H2O)63+(aq)  Al(OH)(H2O)52+(aq) + H+(aq) Acid Conjugate base Proton

  31. Effect of Structure on Acid-Base Properties

  32. Strength of oxyacids • The more oxygen hooked to the central atom, the more acidic the hydrogen. • HClO4 > HClO3 > HClO2 > HClO • Remember that the H is attached to an oxygen atom. • The oxygens are electronegative • Pull electrons away from hydrogen

  33. Cl O H Strength of oxyacids Electron Density

  34. Cl O H Strength of oxyacids Electron Density O

  35. Cl O H Strength of oxyacids Electron Density O O

  36. Cl O H Strength of oxyacids Electron Density O O O

  37. Highly charged metal ions pull the electrons of surrounding water molecules toward them. Make it easier for H+ to come off. Hydrated metals H O Al+3 H

  38. Acid-Base Properties of Oxides • Non-metal oxides dissolved in water can make acids. • SO3 (g) + H2O(l) H2SO4(aq) • Ionic oxides dissolve in water to produce bases. • CaO(s) + H2O(l) Ca(OH)2(aq)

  39. What is the concentration of H3O+ in pure water? • 1.00 x 10–7 M • 7.00 M • 1.00 x 10-14 • 1.00 x 107 M • 7.00 x 10-14 0 of 30

  40. [H+] = 8.26 x 10–5 M, what is the pH of the solution? • 2.16 • 4.10 • 4.08 • 4.083 • 8.024 0 of 30

  41. Which of the following is a conjugate acid/base pair? • HCl/OCl- • H2SO4/SO42- • NH4+/NH3 • H3O+/OH- • none of these 0 of 30

  42. Which of the following indicates the most basic solution? • [H+] = 1 × 10–10 M • pOH =6.7 • [OH–] = 7 × 10–5 M • pH = 4.2 • At least two of the solutions are equally basic. 0 of 30

  43. Calculate the pH of a 0.17 M solution of HOCl, Ka = 3.5 10-8. • 4.11 • 8.23 • 9.89 • 1.00 • 3.77 0 of 30

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